Topic 4.1 Ionic bonding and structure
- Positive ions (cations) form by metals losing valence electrons.
- Negative ions (anions) form by non-metals gaining electrons.
- The number of electrons lost or gained is determined by the electron configuration of an atom.
- The ionic bond is due to electrostatic attraction between oppositely charged ions.
- Under normal conditions, Ionic compounds are usually solids with lattice structures.
Course materials
Class presentation to take notes and put into notebook:
Topic 4.1 Ionic Bonding & Structure
Homework Assignments:
Intermolecular Forces (use Molecule Simulation below)
Formation of Ions
Topic 4.1 Ionic Bonding & Structure
Homework Assignments:
Intermolecular Forces (use Molecule Simulation below)
Formation of Ions
Molecule polarity simulation
Topic 4.2 covalent bonding
- A covalent bond is formed by the electrostatic attraction between a shared pair of electrons and the positively charged nuclei.
- Single, double, and triple covalent bonds involve one, two, and three shared pair of electrons, respectively.
- Bond length decreases and bond strength increases as the number of shared electrons increases.
- Bond polarity results from the difference and electronegativities of the bonded atoms.
Course materials
Class presentation to take notes and put into notebook:
Topic 4.2 Covalent Bonding
Homework:
Bonding Activity
Topic 4.2 Covalent Bonding
Homework:
Bonding Activity
Ionic vs covalent bonding tutorial
Topic 4.3 covalent structures
- Lewis (electron dot) structure show all the valence electrons in a covalently bonded species.
- The octet rule refers to the tendency of atoms to gain a valence shell with a total of eight electrons.
- Some atoms like, Be and B, might form stable compounds with incomplete octets of electrons
- Resonance structures occur when there's more than one possible position for a double bond in a molecule.
- Shapes of species are determined by the repulsion of electron pairs according to the valence shell electron pair repulsion (VSEPR) theory
- Carbon and silicon form covalent network (giant covalent) structures.
Course materials
Class presentation to take notes and put into notebook:
Topic 4.3 Covalent Structures
Homework:
Construct a Lewis Structure
Modeling Molecular Shapes
Topic 4.3 Covalent Structures
Homework:
Construct a Lewis Structure
Modeling Molecular Shapes
molecule polarity tutorial
drawing lewis structures tutorial: basic structures
Drawing lewis structures tutorial: resonance structures
Topic 4.4
- Intermolecular forces include London (dispersion) forces, dipole-dipole forces, and hydrogen bonding.
- The relative strengths of these interactions are London(dispersion) forces < dipole-dipole forces < hydrogen bonds.
Course Materials
Class presentation to take notes and put into notebook:
Topic 4.4 Intermolecular Forces
Homework:
Intermolecular Forces Activity
Topic 4.4 Intermolecular Forces
Homework:
Intermolecular Forces Activity
Intermolecular forces tutorial
Topic 4.5 Metallic Bonding
- A metallic bond is the electrostatic attraction between a lattice of positive ions and delocalized electrons.
- The strength of the metallic bond depends on the charge of ions in the radius of the metal ion.
- Alloys usually contain more than one metal and have enhanced properties.
Course materials
Class presentation to take notes and put into notebook:
Topic 4.5 Metallic Bonding
Homework:
Metallic Bonding Video
Topic 4.5 Metallic Bonding
Homework:
Metallic Bonding Video
Study guides for unit exam
Application and Skills Checklist (IB Specific): Chemical Bonding & Structure Study Guide
Chemical Bonding & Structure Practice Questions: Topic 4 Practice Questions
Chemical Bonding & Structure Practice Questions: Topic 4 Practice Questions